Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?(1 point) Responses The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid. The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid. The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid. The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid. A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium. A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium. If the initial concentration of each acid is the same, then acetic acid will produce more H3O+ ions than hydrochloric acid.

The correct statement about hydrochloric acid and acetic acid is:

**The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.**

Hydrochloric acid (HCl) is a strong acid that completely dissociates in water, leading to a very high dissociation constant. In contrast, acetic acid (CH₃COOH) is a weak acid that only partially dissociates, resulting in a much lower dissociation constant. Therefore, the first statement is true, while the others are not correct in the context given.

- The second statement about pH is not universally correct because it depends on the concentrations of the acids.
- The third statement is also not necessarily correct, as the concentration of solute at equilibrium will depend on the extent of dissociation relative to initial concentrations.
- The fourth statement is incorrect because the strong acid will produce more H₃O⁺ ions than the weak acid if their initial concentrations are the same.